Semimetallic silicon can be made by the electrolysis of molten SiO2. (a) What mass of Si is formed by passing a current of 8.03 A through molten SiO2 for 2.60 days? The unbalanced chemical reaction representing this electrolysis is shown below.

Q: Chromium can be electroplated from aqueous potassium dichromate, with the reduction shown below. If…

A: Given data Current (i) = 6 A Voltage (v) = 4.5 V Volume of K2Cr2O7 = 215 mL Concentration of K2Cr2O7…

Q: A constant current is passed through an electrolytic cell containing molten MgCl2 for 12 hours. If…

A:

Q: A galvanic cell Cr(s)|Cr2+(aq) || Sn2+(aq)|Sn(s) is constructed using a completely immersed Cr…

A: Cr(s) is undergoing oxidation to Cr2+(aq) and Sn2+(aq) undergoing reduction to Sn(s) half-reactions…

Q: Determine the molar mass (amu) of Metal (M) if it took 1.68 minutes for a current of 1.08 A to plate…

A: The metal will come out as M3++3e-= M . We can conclude from here that 3 moles of electrons are…

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A:

Q: What mass of aluminum metal can be produced per hour in the electrolysis of a molten aluminum salt…

A: The mass of aluminum metal can be produced per hour in the electrolysis of a molten aluminum salt by…

Q: In an electrolysis of a solution containing Ni2+ (aq), metallic Ni(s) deposits on the cathode. Using…

A: (a) Current is the amount of charge flowing per unit time. If I is the current(in A) andt is the…

Q: You have 1.0 M solutions of Al(NO3)3 and AgNO3 along with Al and Ag electrodes to construct a…

A: A voltaic cell is an electrochemical cell that uses a chemical reaction to produce electrical…

Q: What mass of zinc (in grams) is deposited at the cathode when a current of 9.8 amperes passes…

A: According to the electrochemistry Mass of substance deposited,  W = ZCt Where,   t = time in second…

Q: A galvanic cell with a voltage of 1.3 V utilises the reaction: Zn + Cu2+ →→ Cu + Zn2+, as a source…

A: Given: The cell voltage is 1.3 V. The amount of Cu and Zn used is 6.3 g and 11 g, respectively.

Q: Consider the electrolysis of tin (II) sulphate during which tin is deposited at one electrode and…

A: A numerical problem based on electrolysis, which is to be accomplished.

Q: A constant current of 0.445 A is passed through an electrolytic cell containing molten BaCl2 for…

A: The reaction is, Ba2+ + 2e- ---> Ba(s) From this reaction, we can conclude that 2 mol of…

Q: A lead storage battery delivers a current of 6 A for one hour and 22 minutes at a voltage of 12 V.…

A: The electrical energy which is generated in the lead storage battery will be equivalent to the…

Q: How long would it take to deposit 9.38 g of copper (molar mass 63.55 g/mol) at the cathode of an…

A: Faraday's law states that the amount of chemical change that is produced by passing a current to an…

Q: (a) The discharge reaction for a zinc-manganese dioxide battery can be represented as: Zn(s) +…

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Q: The element hafnium, Hf, is used in control rods for nuclear reactors and as an insulator for…

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Q: An electrolysis cell that deposits gold (from Au*(a)) operates for 15 minutes at a current of 2.30…

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Q: Molten CaCl, can be electrolyzed to form metallic Ca. For what duration should an electrolysis be…

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Q: Chromium can be electroplated from aqueous potassium dichromate, with the reduction shown below. If…

A: a) 215 ml  ofb1.25  potassium  means (1.25/1000)×215 = 0.26 mol of potassium dichromate.   From the…

Q: 3. The passage of a current of 0.750 A for 25.0 min deposited 0.369 g of copper from a Cuso,…

A: The Faraday's laws are the main concepts of electrochemistry.  The first law shows  the connection…

Q: The following cell Ag | Ag+(0.10M) || Ag+(1.0M) | Ag is a concentration cell and is capable of…

A:

Q: Electroplating is a way to coat a complex metal object with a very thin (and hence inexpensive)…

A: We have given that Current (I) = 240 mA = 0.24 A Time (t) = 55 sec Equivalent weight of silver =…

Q: Gold can be plated out of a solution containing Au3+ according to the half-reaction:Au3+(aq) + 3…

A: It is given that gold is plated for 25 minutes and the current is of 5.5 A and the half-reaction is…

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A: Galvanic cell converts chemical energy into electrical energy. Here Zn rod is dipped in ZnSO4…

Q: Determine the molar mass (amu) of Metal (M) if it took 2.95 minutes for a current of 1.8 A to plate…

A:

Q: In the electrolysis of an acid solution, oxygen can be produced by the following half-reaction:…

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Q: Tin-plated steel is used for "tin" cans. Suppose that in the production of sheets of tin-plated…

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Q: Aluminum metal can be made from aluminum(III) ions by electrolysis. What is the half-reaction at the…

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Q: (a) How many coulombs are required to plate a layer of nickel metal 0.125 mm thick on a coin with a…

A: (a) Calculate the volume of Nickel for plating the coin: The shape of nickel after electroplating…

Q: The electrolysis of AℓCℓ3 at high temperature produces aluminium metal. If a constant electrical…

A: Given:  Current (I) = 10 x 103 Amp  Time(t) = 1 hour = 3600 sec

Q: Question attached

A: Current is equal to the flow of charge per unit of time. It is denoted by I. Its SI unit is ampere.…

Q: In an electrolysis of a solution containing Ni^2+ (aq), metallic Ni (s) deposits on the cathode.…

A:

Q: Suppose somebody in the laboratory doesn’t quite turn off the current in an electrolysis cell so…

A: The relation between charge and time is shown below: Q = It where; Q = charge I = current t = time

Q: How many amperes of current needs to be passed through molten Sodium chloride (NaCl) to produce 2.1…

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Q: • Part A A lead-acid battery uses a redox reaction in which lead(0) and lead(IV) are both converted…

A: The reaction given is, => Given: Time passed = 5.00 hours = 5 × 60 × 60 = 18000 s…

Q: Suppose that a machine part requires 400 mg of copper to provide a coating that is thick enough for…

A: Given data,Current=0.5ATime=10min=10×60s=600s

Q: A current of 200 A flows for 22.0 hours at an anode where the reaction occurring is Mn2*(aq) +…

A: Interpretation- To determine the mass(in Kg) of MnO2  is deposited on this anode when a current of…

Q: 2. Tin-plated steel is used for tin cans. If the production of sheets of tin-plated steel requires…

A: Formulas used : I = q/t     where I is the current in amperes                            q is the…

Q: The electrolysis of an aqueous solution of potassium iodide, KI, results in the formation of…

A: Electrolysis: It is a chemical reaction that occurs when an electric current is conducted through a…

Q: Molten CaCl₂ can be electrolyzed to form metallic Ca. For what duration should an electrolysis be…

A: Faraday's first law :-  It states that, the amount of the substance deposited at the electrode is…

Q: A lead storage battery delivers a current of 6 A for one hour and 22 minutes at a voltage of 12 V.…

A: (a)

Q: (a) In the electrolysis of aqueous NaNO2, how many liters of O2(g) (at STP) are generated by a…

A: Interpretation -  In the electrolysis of aqueous NaNO2, how many liters of O2(g) (at STP) are…

Q: d) For a thermodynamic process, when ΔΗsys > 0, and ΔSsys7, pH<7, or pH-7)

A: d) For a thermodynamic process, the expression for change in Gibbs free energy is related to change…

Q: Cell 1 Cell 2 Two identical spoons were electroplated with Ag or Cd through the use of the…

A: given - electroplating diagram for Ag and Cd

Q: The amount of lactic acid, HC3H5O3, produced in a sample of muscle tissue was analyzed by reaction…

A: In case of lactic acid the no. of moles of acid is equal to the no. of moles of hydroxide ion that…

Q: The passage of a current of 0.750 A for 25.0 min deposited 0.369 g of copper from a CuSO, solution.…

A:

Q: Consider a simple galvanic cell consisting of two beakers connected by a salt bridge. One beaker…

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Q: When a lead acid car battery is recharged by the alternator, it acts essentially as an electrolytic…

A: According to the Faraday's law of electrolysis, the mass of Substance liberated or deposited at any…

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.